Question

I have a special ideal balloon. This balloon does not exert any pressure on the gas inside it. I started by taking the balloon and inflating it to 4 L on Brooklyn Ny last night. The weather channel said that the temperature was 45.0 degree Celsius, and the pressure was 50.27 mm of Hg.

First i took this balloon scuba diving and went down to a depth of 100 ft where the pressure is 7 atm. And the temperature is 52.2 Celsius. What is the volume of the balloon?

Answer 1

Using ideal gas law PV = nRT Where p is pressure V is the volume n is the number of moles R is the gas constant T is the temperature First solve for the number of moles
N = (50.27 mmHg) ( 4 L) / [( 760 mmHg)( 22.414 L/mol)/ 273.15 K)] ( 45 + 273.15 K)
N = 0.01013 moles
Then solving for the volume
V = nRT / P
V = 0.01013 moles [ ( 1 atm)( 22.414 L/mol)/ 273.15 K)] ( 52.2 + 273.15 K) / 7 atm

V = 0.03865 L